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Kinetics and Equilibrium

Total questions: 40

Worksheet time: 42mins

Name
Class
Date
1.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
2.
The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Which pathway is slower and why?
a)
Red, because the activation energy is larger
b)
Blue, because the activation energy is lower
c)
both reaction progress at the same rate
3.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of particle collisions

4.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
5.
How do catalysts increase the rate of reaction?
a)
The frequency of collisions is the increased
b)
the activation energy is lowered
c)
the energy of collisions is increased
d)
Both the frequency and energy of collisions is increased
6.

Which statement correctly describes an endothermic chemical reaction?

a)

The products have lower potential energy than the reactants, and the ΔH is positive

b)

The products have lower potential energy than the reactants, and the ΔH is negative

c)

The products have higher potential energy than the reactants, and the ΔH is positive

d)

The products have higher potential energy than the reactants, and the ΔH is negative

7.

Which balanced equation represents an endothermic reaction?

a)

N2(g) + 3H2(g) --> 2NH3(g)

b)

N2(g) + O2(g) --> 2NO(g)

c)

CH4(g) + 2O2(g) --> CO2(g) + 2H2O(l)

d)

C(s) + O2(g) --> CO2(g)

8.

Which statement about a system at equilibrium is true?

a)

The forward reaction rate stops and the reverse reaction rate continues

b)

The forward reaction rate is greater than the reverse reaction rate.

c)

The forward reaction rate is less than the reverse reaction rate

d)

The forward reaction rate is equal to the reverse reaction rate.

9.

The potential energy diagram below represents a reaction.


Which arrow represents the activation energy of the forward reaction

a)

A

b)

B

c)

C

d)

D

10.

Which statement best explains the role of a catalyst in a chemical reaction?

a)

A catalyst changes the kinds of products produced

b)

A catalyst provides an alternate reaction pathway that requires less activation energy

c)

A catalyst limits the amount of reactants used

d)

A catalyst is added as an additional reactant and is consumed but not regenerated

11.

Which sample has the lowest entropy?

a)

1 mole of KNO3(l)

b)

1 mole of KNO3(s)

c)

1 mole of KNO3(aq)

d)

1 mole of KNO3(g)

12.

Given the balanced equation


Which statement best describes this proces

a)

It is endothermic and entropy decreases

b)

It is endothermic and entropy increases

c)

It is exothermic and entropy decreases

d)

It is exothermic and entropy increases

13.

Systems in nature tend to undergo changes toward

a)

lower energy and lower entropy

b)

lower energy and higher entropy

c)

higher energy and lower entropy

d)

higher energy and higher entropy

14.
If a catalyst is added to a system at equilibrium and the temperature and pressure remain constant, there will be no effect on the
a)
rate of the forward reaction
b)
activation energy of the reaction
c)
rate of the reverse reaction
d)
heat of reaction
15.
Adding a catalyst to a chemical reaction changes the rate of reaction by causing
a)
a decrease in the activation energy
b)
an increase in the activation energy
c)
a decrease in the heat of reaction
d)
an increase in the heat of reaction
16.
Which interval represents the heat of reaction for the reaction?
a)
A
b)
B
c)
D
d)
E
17.
Interval C in this potential energy diagram could be changed by adding a ________?
a)
Cookies
b)
More energy
c)
Catalyst
d)
Changing the temperature
18.
Which term refers to the difference between thepotential energy of the products and the potential energy ofthe reactants for any chemical change?
a)
heat of deposition
b)
heat of fusion
c)
heat of reaction
d)
heat of vaporization
19.

Given the equation representing a reaction at equilibrium:

N2(g) + 3H2(g) --> 2NH3(g) + energy

Which change causes the equilibrium to shift to the right?

a)

decreasing the concentration of H2(g)

b)

decreasing the pressure

c)

increasing the concentration of N2(g)

d)

increasing the temperature

20.
Given the reaction at equilibrium:
N2(g) + O2(g) ↔ 2NO(g)
As the concentration of N2(g) increases, the concentration of O2(g) will
a)
decrease
b)
increase
c)
remain the same
21.

For the reaction SO2 + O2 <−> SO3

If the equilibrium shifts to the left, the concentration of SO3 will ___________.

a)

Increase

b)

Decrease

c)

Stay the same

22.

For the reaction SO2 + O2 <−> SO3

If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.

a)

To the left

b)

To the right

c)

To the left and right

d)

Neither left nor right

23.
Which list of the phases of H2O is arranged in order of increasing entropy?
a)
ice, steam, and liquid water
b)
ice, liquid water, and steam
c)
steam, liquid water, and ice
d)
steam, ice, and liquid water
24.
 Given the equation representing a reaction at equilibrium:
2SO2(g) + O2(g) <--> 2SO3(g) +HEAT
Which change causes the equilibrium to shift to the right?
a)
adding a catalyst
b)
 adding more O2(g)
c)
decreasing the pressure
d)
increasing the temperature
25.

Given the equation representing a system at equilibrium:

N2(g) + 3H2(g) <--> 2NH3 (g) + ENERGY

Which changes occur when the temperature of this system is decreased?

a)

The concentration of H2(g) increases and the concentration of N2(g) increases.

b)

The concentration of H2(g) decreases and the concentration of N2(g) increases.

c)

The concentration of H2(g), N2(g), and NH3(g) decreases.

d)

The concentration of H2(g) and N2(g) decreases and the concentration of NH3(g) increases.

26.
Given the equation representing a closed system:
N2O4(g) <--> 2NO2(g)
Which statement describes this system at equilibrium?
a)
The volume of the NO2(g) is greater than the volume of the N2O4(g).
b)
The volume of the NO2(g) is less than the volume of the N2O4(g).
c)
The rate of the forward reaction and the rate of the reverse reaction are equal.
d)
The rate of the forward reaction and the rate of the reverse reaction are unequal.
27.
Which term is defined as a measure of the disorder of a system?
a)
heat
b)
entropy
c)
kinetic energy
d)
activation energy
28.

The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Which pathway is faster and why?

a)

Red, because the activation energy is larger

b)

Blue, because the activation energy is lower

c)

both reaction progress at the same rate

29.

What letter represents the potential energy of the reactants?

a)

A

b)

B

c)

C

d)

D

30.

What letter represents the potential energy of the products?

a)

A

b)

F

c)

D

d)

E

31.

What letter represents the potential energy of the activated complex?

a)

B

b)

D

c)

F

d)

E

32.

What letter represents the heat of the reaction (ΔH)?

a)

A

b)

B

c)

C

d)

D

33.

What letter represents the activation energy of the forward reaction?

a)

A

b)

B

c)

C

d)

D

34.

What letter represents the activation energy of the reverse reaction?

a)

E

b)

F

c)

A

d)

D

35.

Is this reaction endothermic or exothermic?

a)

endothermic

b)

exothermic

36.

Which sample has the highest entropy?

a)

1 mole of KNO3(l)

b)

1 mole of KNO3(s)

c)

1 mole of KNO3(aq)

d)

1 mole of KNO3(g)

37.

Given the equation representing a reaction at equilibrium:

N2(g) + 3H2(g) --> 2NH3(g) + energy

Which change causes the equilibrium to shift to the left?

a)

decreasing the concentration of H2(g)

b)

decreasing the pressure

c)

increasing the concentration of N2(g)

d)

decreasing the temperature

38.

Which list of the phases of H2O is arranged in order of decreasing entropy?

a)

ice, steam, and liquid water

b)

ice, liquid water, and steam

c)

steam, liquid water, and ice

d)

steam, ice, and liquid water

39.

Which one of these types of compounds tend to have a faster rate of reaction?

a)

Ionic Compounds

b)

Covalent Compounds

c)

Polar Covalent Compounds

40.

Freebie Question..select Answer Choice 1 for free points!

a)

Free points

b)

No, I want to get a bad grade

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